Chapter_5 Sep_19 Lecture_13.pptx

Lattice energy depends on the magnitudes of the

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Lattice energy depends on the magnitudes of the charge and on the distance between them = charges = distance between ion centers = 8.99x10 9 J m C –2 LE increases as: -- charges increase -- size of ions decrease (d) Lattice Energy

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Lattice Energy Same charge , larger radius (d) , smaller LE
Lattice Energy similar radius (d) , larger charge , greater LE

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Lattice Energy Which LE is greater? Consider charge first! Larger charge, greater LE . If same charge, then use radius to break the ties. K + F Ca 2+ Br Na + F Mg 2+ O 2− Ca 2+ I What about KF and NaF? Which one has larger LE? NaF has larger LE because Na + has smaller radius than K + , thus smaller
What Else LE Tells Us Lattice energy is a measure of an ionic compound’s stability. -the greater LE, the stronger the interactions in the ionic substance -the greater LE, the higher the melting point (solid → liquid)

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5.4 Naming Ions and Ionic Compounds A monatomic cation is named by adding the word ion to the name of the element K + is potassium ion Ca 2+ is calcium ion A monatomic anion is named by changing the ending of the element’s name to – ide. Cl is chloride O 2– is oxide Some metals can form cations of more than one possible charge. Mn 2+ : manganese(II) ion Mn 3+ : manganese(III) ion Mn 4+ : manganese(IV) ion Which one is manganese chloride, MnCl 2 , MnCl 3 , or MnCl 4 ?
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• Ion, Formulas of Ionic Compounds

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